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  2. Dipolar compound - Wikipedia

    en.wikipedia.org/wiki/Dipolar_compound

    In organic chemistry, a dipolar compound or simply dipole is an electrically neutral molecule carrying a positive and a negative charge in at least one canonical description. In most dipolar compounds the charges are delocalized . [ 1 ]

  3. Chemical polarity - Wikipedia

    en.wikipedia.org/wiki/Chemical_polarity

    Note that the dipole moments drawn in this diagram represent the shift of the valence electrons as the origin of the charge, which is opposite the direction of the actual electric dipole moment. The bond dipole moment [5] uses the idea of electric dipole moment to measure the polarity of a chemical bond within a molecule. It occurs whenever ...

  4. Coordinate covalent bond - Wikipedia

    en.wikipedia.org/wiki/Coordinate_covalent_bond

    In coordination chemistry, a coordinate covalent bond, [1] also known as a dative bond, [2] dipolar bond, [1] or coordinate bond [3] is a kind of two-center, two-electron covalent bond in which the two electrons derive from the same atom. The bonding of metal ions to ligands involves this kind of interaction. [4]

  5. Non-covalent interaction - Wikipedia

    en.wikipedia.org/wiki/Non-covalent_interaction

    A hydrogen bond (H-bond), is a specific type of interaction that involves dipoledipole attraction between a partially positive hydrogen atom and a highly electronegative, partially negative oxygen, nitrogen, sulfur, or fluorine atom (not covalently bound to said hydrogen atom). It is not a covalent bond, but instead is classified as a strong ...

  6. N,N'-Dicyclohexylcarbodiimide - Wikipedia

    en.wikipedia.org/wiki/N,N'-Dicyclohexylcarbodiimide

    N,N′-Dicyclohexylcarbodiimide (DCC or DCCD) [1] is an organic compound with the chemical formula (C 6 H 11 N) 2 C. It is a waxy white solid with a sweet odor. Its primary use is to couple amino acids during artificial peptide synthesis. The low melting point of this material allows it to be melted for easy handling.

  7. Polarizability - Wikipedia

    en.wikipedia.org/wiki/Polarizability

    The polarizability of an atom or molecule is defined as the ratio of its induced dipole moment to the local electric field; in a crystalline solid, one considers the dipole moment per unit cell. [1] Note that the local electric field seen by a molecule is generally different from the macroscopic electric field that would be measured externally.

  8. Chemical species - Wikipedia

    en.wikipedia.org/wiki/Chemical_species

    The chemical species can be an atom, molecule, ion, or radical, with a specific chemical name and chemical formula. [ 2 ] In supramolecular chemistry , chemical species are structures created by forming or breaking bonds between molecules, such as hydrogen bonding , dipole-dipole bonds , etc. [ 3 ] These types of bonds can determine the ...

  9. Thiol - Wikipedia

    en.wikipedia.org/wiki/Thiol

    The S−H bond in thiols is weak compared to the O−H bond in alcohols. For CH 3 X−H, the bond enthalpies are 365.07 ± 2.1 kcal/mol for X = S and 440.2 ± 3.0 kcal/mol for X = O. [ 21 ] Hydrogen-atom abstraction from a thiol gives a thiyl radical with the formula RS • , where R = alkyl or aryl.